Name:______Date:______Period:______

Standards Review

2a. Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form ionic bonds.

Description

In the localized electron model, a covalent bond appears as a shared pair of electrons contained in a region of overlap between two atomic orbitals. Atoms (usually nonmetals) of similar electronegativities can form covalent bonds to become molecules.

In a covalent bond, therefore, bonding electron pairs are localized in the region between the bonded atoms. In metals valence electrons are not localized to individual atoms but are free to move to temporarily occupy vacant orbitals on adjacent metal atoms. For this reason metals conduct electricity well.

When an electron from an atom with low electronegativity (e.g., a metal) is removed by another atom with high electronegativity (e.g., a nonmetal), the two atoms become oppositely charged ions that attract each other, resulting in an ionic bond.

Chemical bonds between atoms can be almost entirely covalent, almost entirelyionic, or in between these two extremes. The triple bond in nitrogen molecules(N2) is nearly 100 percent covalent. A salt such as sodium chloride (NaCl) has bonds that are nearly completely ionic. However, the electrons in gaseous hydrogenchloride are shared somewhat unevenly between the two atoms. This kind of bond is called polar covalent.(Note that elements in groups 1, 2, 16, and 17 in the periodic table usually gain or lose electrons through the formation of either ionic or covalent bonds, resultingin eight outer shell electrons. This behavior is sometimes described as “the octet rule.”)

Vocabulary

ORBITAL OVERLAP

COVALENT BOND

MOBILE ELECTRONS IN METALS

ELECTROSTATIC ATTRACTION

POLARITY OF A COVALENT BOND (describe similarities and differences between polar and nonpolar covalent bond)

OCTET RULE

Practice Problems

  1. When elements from group 1 (1A) combine with elements from group 17 (7A), they produce compounds. Which of the following the correct combining ratio is between group 1 (1A) elements and group 17 (7A) elements?

A. 1:1 B. 1:2

C. 2:1 D. 3:2

  1. The bonds in BaO are best described as-

A. covalent, because valence electrons are shared

B. covalent, because valence electrons are transferred

C. ionic, because valence electrons are shared

D. ionic, because valence electrons are transferred

  1. The strength of an atom’s attraction for the electrons in a chemical bond is the atom’s-

A. electronegativity C. heat of reaction

B. ionization energy D. heat of formation

  1. The chemical bond between which two atoms is most polar?

A. C–N C. S–Cl

B. H–H D. Si–O

  1. When cations and anions join, they form what kind of chemical bond?

A. ionic B. hydrogen

C. metallic D. covalent

  1. Which of the following atoms has six valence electrons?

A. magnesium (Mg) B. silicon (Si)

C. sulfur (S) D. argon (Ar)

2b. Students know chemical bonds between atoms in molecules such as H2, CH4, NH3, H2CCH2, N2, Cl2, and many large biological molecules are covalent.

Description

Organic and biological molecules consist primarily of carbon, oxygen, hydrogen,and nitrogen. These elements share valence electrons to form bonds so that the outer electron energy levels of each atom are filled and have electron configurations like those of the nearest noble gas element. (Noble gases, or inert gases, are in the last column on the right of the periodic table.)

For example, nitrogen has one lone pair and three unpaired electrons and therefore can form covalent bonds with three hydrogen atoms to make four electron pairs around the nitrogen.

Carbon has four unpaired electrons and combines with hydrogen, nitrogen, and oxygen to form covalent bonds sharing electron pairs.

The great variety of combinations of carbon, nitrogen, oxygen, and hydrogen make it possible, through covalent bond formation, to have many compounds from just these few elements.

List four macromolecules and their monomers INCLUDE a visual description

Vocabulary

ORGANIC MOLECULES

VALENCE ELECTRONS

ENERGY LEVELS

ELECTRON CONFIGURATION

NOBLE GASES

INERT

UNPAIRED ELECTRONS

SHARED PAIRS OF ELECTRONS

BALL AND STICK MODELS

Practice Problems

  1. The diagram below shows the structure of a brain chemical called acetylcholine:

Based on the nature of the elements making up acetylcholine, the bonds present in the compound are most likely…

A. nuclear C. hydrogen

B. metallic D. covalent

2c. Students know salt crystals, such as NaCl, are repeating patterns of positive and negative ions held together by electrostatic attraction

Description

The energy that holds ionic compounds together, called lattice energy is caused by the electrostatic attraction of cations, which are positive ions, with anions, which are negative ions. To minimize their energy state, the ions form repeating patterns that reduce the distance between positive and negative ions and maximize the distance between ions of like charges.

Prepare a labeled diagram to illustrate the description.

Vocabulary

CATIONS

ANIONS

CRYSTAL LATTICE

IONIC COMPOUNDS

LATTICE ENERGY

SALT, NaCl

  1. Which of the following elements can form an anion that contains 54 electrons, 74 neutrons, and 53 protons?

2d. Students know the atoms and molecules in liquids move in a random pattern relative to one another because the intermolecular forces are too weak to hold the atoms or molecules in a solid form

In any substance at any temperature, the forces holding the material together are opposed by the internal energy of particle motion, which tends to break the substance apart. In a solid, internal agitation is insufficient to overcome intermolecular or inter-atomic forces.

When enough energy is added to the solid, the kinetic energy of the atoms and molecules increases sufficiently to overcome the attractive forces between the particles, and they break free of their fixed lattice positions. This change, called melting, forms a liquid, which is disordered and non-rigid. The particles in the liquid are free to move about randomly although they remain in contact with each other. The particles in a gas are free to move about randomly

Vocabulary

PARTICLE MOTION

LIQUIDS

SOLIDS

GASES

INTERMOLECULAR FORCES OF ATTRACTION [IMF]

KINETIC ENERGY

MELTING

BOILING

  1. Which change in state would involve a decrease in the intermolecular force of attraction holding the water particles together?

A. H2O(s) → H2O( ) C. H2O(g) → H2O(s)

B. H2O(g) → H2O(l) D. H2O(l) → H2O(s)

2e. Students know how to draw Lewis dot structures

Description

A Lewis dot structure shows how valence electrons and covalent bonds are arranged between atoms in a molecule. Teachers should follow the rules for drawing Lewis dot diagrams provided in chemistry textbook. Students should be able to use the periodic table to determine the number of valence electrons for each element in Groups 1 through 3 and 13 through 18. Carbon, for example, would have four valence electrons. Lewis dot diagrams represent each electron as a dot or an x placed around the symbol for carbon, which is C. A covalent bond is shown as a pair of dots, or x’s, representing a pair of electrons or a line. For example, a Lewis dot diagram for methane, which is CH4, would appear as shown in Figure 3.

Lewis dot diagrams provide a method for predicting correct combining ratios between atoms and for determining aspects of chemical bonds, such as whether they are covalent or consist of single, double, or triple bonds.

The illustration below shows two atoms of a fictitious element (M) forming a diatomic molecule.

  1. What type of bonding occurs between these two atoms?

A. covalent B. ionic

C. nuclear D. polar

Chemistry Standard Set 21